Rate Constant and Order of Reactions
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I need help understanding how to determine orders of reaction:
1. For a first order reaction w/rate constant of .35 sec-1, the percent starting material remaining after 25 sec is:
2. Rate data for the reaction 2 NOBr (g)->; 2 NO (g) + Br2 (g) follows:
[NOBr] Rate (mol L-1 s-1)
.0450 1.62 x 10-3
.0310 7.69 x 10-4
.0095 7.22 x 10-5
The overall order for the reaction is:
3. For the reaction 2 A ->; 1B, the rate constant is 6.00 x 10-3 (M min)-1. The overall order of reaction is:
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Solution Summary
The solution identifies what order of reaction each scenario is and also why such order is chosen. Full explanations on reaction kinetics and rate constants.
Solution Preview
To understand the problems I go with the assumption that you have a basic understanding of the reaction kinetics.
1. For solving this problem we use the following equation in first order:
ln[A]t - ln[A]0 = ln[A]t/ ln[A]0 = -kt
where ln[A]t and ln[A]0 are ...
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